Final answer:
Without the concentration of Ca(OH)2, the exact volume of 3.35×10^-3 M HCl required to neutralize 10 mL of Ca(OH)2 cannot be determined; however, the calculation would involve stoichiometry and the molar ratio from the chemical equation.
Step-by-step explanation:
To determine the volume of 3.35×10-3 M HCl needed to neutralize 10.0 mL of a saturated Ca(OH)2 solution, we need to apply the concept of stoichiometry. For every mole of Ca(OH)2, two moles of HCl are needed for neutralization because of the chemical equation Ca(OH)2 + 2HCl → CaCl2 + 2H2O.
The concentration and volume of Ca(OH)2 are not provided directly, so we cannot calculate the required volume of HCl. However, typically this would be done by calculating the number of moles of Ca(OH)2 (using its concentration and volume), doubling that number (to account for the 2:1 ratio in the reaction), and then using the molarity of HCl to find the required volume.